+ pH and KineticsThe iodate ion, IO3 is reduced by sulfite. SO², according to thefollowing net ionic equation:IO, (aq) + 350,² (aq) + (aq) + 350,² (aq)Part Afound to be first order in IO3, first order in SO3²and first order in H+.If [103] z. [SO₂²]y, and [H¹] = Z, what is the rate law for the reaction terms of z, y, and 2 and the rate constant k?Express the rate in terms of k, z▸ View Available Hint(s)and 2 (e.g., kxy^3z^2).|VL | ΑΣΦThe reactionrate =Submit16 of 43 >Review | Constants | Periodic Table

First we need to write the rate law of given reaction as per orders . Then we would plug the values…

The reaction is found to be first order in 10s first order in SO3² and first order in H¹. If [10₂]=z. [S0₂² 1 y. and H=2, what is the rate law for the reaction in terms of z. y. and 2 and the rate constant k? Express the rate in terms of k, z, y, and z (e.g., kxy^3z^2). View Available Hintis)

The reaction is found to be first order in 10s first order in SO3² and first order in H¹. If [10₂]=z. [S0₂² 1 y. and H=2, what is the rate law for the reaction in terms of z. y. and 2 and the rate constant k? Express the rate in terms of k, z, y, and z (e.g., kxy^3z^2). View Available Hintis)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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20.) A generic reaction has the rate law rate = k[A]2[B]0. What [A], in moles per liter, will be required to give a rate of = 0.383 M/s when the [B] = 0.181 M? The value of the rate constant is 0.344. Do not include units. Your Answer:
Propose a reaction pathway consisting of only a unimolecular or bimolecular steps for the 2A+B-->C+D that is consistent with the rate law rate=k(A)(B). Make sure you label which step is the rate determining step and prove that your proposed mechanism gives both the overall reaction and overall rate law. Explain the assumptions you must make in order for your mechanism to be consistent with the actual rate law.
4. Consider three hypothetical reactions of the type A → products. One of the reactions is zeroth order, one is first order, and one is second order. If they all have the same numerical value of the rate constant k (in units of M s ¹, s and M¹s¹, -1 -1 9 respectively), what must be the initial concentration [A]o if the half-lives are equal for a) the zeroth- and first-order reactions, b) the zeroth- and second-order reactions, and c) the first- and second-order reactions.
The rate of a certain reaction is given by the following rate law: rate =k N, O, Use this information to answer the questions below. olo What is the reaction order in N,? |x10 18 Ar What is the reaction order in 03? What is overall reaction order? At a certain concentration of N, and 03, the initial rate of reaction is 0.780 M / s. What would the initial rate of the reaction be if the concentration of N, were halved? Round M S your answer to 3 significant digits. The rate of the reaction is measured to be 5.0 x 103M/s when [N2] = 1.1 M and [03] = 1.1 M. Calculate the value of - 3 -1 k = |M •S the rate constant. Round your answer to 2 significant digits.
5. You studied the chemical reaction, 2NO2(g) → 2NO(g) + O2(g), at 25°C by monitoring the concentration of NO2(g) as a function of time and constructed the following graph. y= 0.5408x + 125.0 R2=0.998 Time (s) What is the rate constant for this reaction at 25°C? Include the proper units. (W/T) [(3)ONI/T
The following reaction is observed to be second order with respect to NO and first order with respect to Br2. Br2 (g) + 2NO (g) --> 2NOBr (g)
9. The reaction 3C A + 2B occurs in one step in the gas phase. In each blank below, write the exponent of the concentration in the FORWARD rate law or write none if that concentration does not appear in the rate law. [A] ........... [B] .......... [C] ...........
Suggest a mechanism behind the reaction NO(g) + Cl2(g) à NOCl(g) + Cl(g) with the rate law rate = k [NO]2 [Cl2] This reaction cannot be a one step reaction because of its rate law. It is therefore a multistep reaction, where the slow step represents a reaction between 2 molecules of NO with one molecule of Cl2 (slow) 2NO + Cl2 à ………. (fast). à ………… NO + Cl2. à NOCl + Cl
For the reaction: NO (g) + O3 (g) ---> NO2 (g) + O2 (g) the value of A= 8.7 x 1012 s-1 and Ea = 63 kJ/mol. What is the value of the rate constant k for the reaction at 75oC? Enter your answer in units of s-1 to 2 significant figures. Enter your answer in the format: a.b x10^m, where a.b and m are the appropriate numbers based on your calculation.
The rate of a certain reaction was studied at various temperatures. The table shows temperature (7) and rate constant (k) data collected during the experiments. Plot the data to answer the questions. What is the value of the activation energy, Ea, for this reaction? E₁ = 122.7 What is the value of the pre-exponential factor (sometimes called the frequency factor), A, for this reaction? A= 1.147 X10¹2 kJ mol-1 Incorrect T(K) 400 420 440 460 480 500 520 540 560 580 k (s-¹) 0.000108 0.000626 0.00310 0.0134 0.0511 0.175 0.547 1.57 4.18 10.4